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Decomposition of Hydrogen Peroxide

Decomposition of Hydrogen Peroxide. Background. The decomposition of hydrogen peroxide in aqueous solution happens very slowly. A catalyst can be used to speed up this reaction. Objectives: Conduct a catalyzed decomposition of hydrogen peroxide.

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Decomposition of Hydrogen Peroxide

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  1. Decomposition of Hydrogen Peroxide

  2. Background • The decomposition of hydrogen peroxide in aqueous solution happens very slowly. • A catalyst can be used to speed up this reaction. • Objectives: • Conduct a catalyzed decomposition of hydrogen peroxide. • Calculate the rate constant k for this reaction. • Determine the rate law for this reaction. • Calculate the activation energy for this reaction.

  3. Materials • Lab quest • Netbook • Gas pressure sensor • Temperature probe • 4 test tubes and test tube holder • Wash bottle/Distilled water • 3 % hydrogen peroxide (0.88M) • 100 mL volumetric flask • Solid potassium iodide • 2 10 mL graduated cylinders • plastic pipettes • 600 mL beaker • Ring stand and clamp • Glass pipette and pipette bulb

  4. Procedure • We will be doing 4 experiments during this lab to determine the rate law of this reaction and the activation energy.

  5. Solution Preparation • We will be using store bought 3%(0.88M) H2O2 • We will need to make 100 mL of a 0.5 M KI solution. • How many grams of KI will we need? (molar mass of KI = 166.01 g/mol) • 8.3 g • In experiment 2 we will be cutting the concentration of our KI in half. • In experiment 3 we will be cutting the concentration of our H2O2 in half

  6. Data Table

  7. Data Analysis

  8. Analysis Questions • Using your data determine the rate law for this reaction, and calculate the average value of k for the 3 experiments. • Determine the average numerical value of k for experiments. • The rate law should have been first order in both KI and H2O2 using this information determine the units for k.

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